What is the final volume after you reach the final temperature? I put 1.73 but the answer is wrong not sure why The initial volume of gas is 1.60 LL , the initial temperature of the gas is 23.0 °C°C , and the system is in equilibrium with an external pressure of 1.2 bar (given by the sum of a 1 bar atmospheric pressure and a 0.2 bar pressure due to a brick that rests on top of the piston). Then, as you did in Exercise 1, you heat the gas slowly until the temperature reaches 48.2 °C

What is the final volume after you reach the final temperature? I put 1.73 but the answer is wrong not sure why The initial volume of gas is 1.60 LL , the initial temperature of the gas is 23.0 °C°C , and the system is in equilibrium with an external pressure of 1.2 bar (given by the sum of a 1 bar atmospheric pressure and a 0.2 bar pressure due to a brick that rests on top of the piston). Then, as you did in Exercise 1, you heat the gas slowly until the temperature reaches 48.2 °C

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.44QE

See similar textbooks

Similar questions

The ideal gas law is theequation of state for an ideal gas. Why cantit be used to determine TpH?
contains 0.550 bar H2(g)0.550 bar H2(g) , 0.491 bar N2(g)0.491 bar N2(g) , and 0.121 bar Ar(g)0.121 bar Ar(g) . Calculate the mole fraction, ?χ , of each of these gases.
Give detailed Solution with explanation needed (no need Handwritten answer)
Consider a container with a frictionless piston that contains a given amount of an ideal gas. If the external pressure is kept constant, the piston will move up or down in response to a change in the internal pressure. The piston will move up if Pint > Pext and vice versa. The piston will stop moving when Pint Pext (the system is equilibrated). = The container has 0.8 mol of an ideal gas initially at 24 °C and the system is in equilibrium with an external pressure of 1.2 bar. The gas is slowly heated to a final temperature of 305 °C. During this process, the piston is allowed to move if necessary to keep the system at equilibrium (that is, the internal pressure is allowed to match the external pressure at all times). The molar heat capacity at constant volume Cum of this ideal gas is 2.5 R. ▼ Part A - Calculate the initial volume of the gas. ▼ Express your answer in m³ with 3 significant figures. The margin of error for this answer is 2%. V₂ = 0.0219 | ΑΣΦ Submit Previous Answers…
A quantity of gas in a piston cylinder has a volume of 0.475 m3 and a pressure of 200 Pa. The piston compresses the gas to 0.272 m3 in an isothermal (constant-temperature) process. What is the final pressure of the gas?
With explanation, Don't use AI.
Part 3: For each of the following questions, refer to the following balanced equation and the Data Table above. Give your answers to the first decimal place if the answer is greater than 1. Otherwise, use exponential format (e. g. 1.23E-10) 2 HgO(s) = 2 Hg(l) + O2(g) f) Determine the value of Keq at 298 K (3 sig. figs.). R = 8.3145 J/moleK g) Determine the value of Grxn at 298 K when the partial pressure of O2(g) is 2.0 atm. Assume the equilibrium constant is Kp. R = 8.3145 J/moleK
2N20(g) + N2H4(9) = 2H20(g) + 3N2(g) If Ke for the above reaction is 36.94 at 197.9 K, what is Kp for the same reaction? (the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0) A Moving to another question will save this response. RQuestion 8 of 31 MacBook Ai %23 %24 % & 7 dolete Y tab F G H K caps lock B shift olt command option control option command is
An ideal gas (the system) is contained in a flexible balloon at a pressure of 1 atm and is initially at a temperature of 20.°C. The surrounding air is at the same pressure, but its temperature is 25°C. When the system has equilibrated with its surroundings, both systems and surroundings are at 25°C and 1 atm. In changing from the initial to the final state, which one of the following relationships regarding the system is correct? Select one: а. DH %3D 0 b. q > 0 C. W > 0 d. DE < 0 e. DE = 0
You measure the total pressure of a system is 228.2kPa (P total). You also find there are 49.9kPa (P1) of Hydrogen and 52.9kPa of Carbon (P2). How much Oxygen (P3) is present?
R = 0.08205 L atm mol-1 K-1 T(K) = T (°C) + 273.15
Given the following chemical equilibrium COCl₂(g)=CO(g) + Cl₂(g), calculate the value of Kc when Kp = 8.32 x 10¹1 at 298 K. (R = 0.08206 L-atm/mol. K). Calculate the value of Kc/10^1¹0.. Answer should have 3 sig figs.